Chemistry flashcards
Unlock all answers in this set
Unlock answers| Who devised the theory of the atom? |
| Democratis |
| Atomic number |
| The number of protons in the nucleus |
| Atomic mass |
| The average weight of the element |
| Mass number |
| The rounded atomic mass, the number of protons and neutrons |
| Nucleus |
| Positively charged center of the atom, contains protons and neutrons |
| Protons |
| Positive particle, in the nucleus |
| Neutrons |
| No charge, in nucleus |
| Electrons |
| Negative, orbit around nucleus |
| Ion |
| Atom with a positive or negative charge |
| Draw an example of a shorthand notation |
Look at notes |
| A neutral atom has ______ number of electrons and protons |
| An equal |
| Isotope |
| Variety of the same element all with different masses |
Find the electron configuration of Calcium (use your tables) |
| 1s22s22p63s23p64s2 |
| How many valence electrons does Nitrogen have? |
| 5 |
What is the charge of the Alikali Metals? Why? |
| +1; because it gives up 1 electron to get 8 valence electrons |
Nonmetals __________ to get 8 valence electrons Metals __________ to get 8 valence electrons |
| Steal electrons; give electrons |
| Period |
| Horizontal rows |
| Group |
| Vertical families |
| What charge do the Alkaline earth metals have? |
| +2 |
| What family is the least reactive? |
| The Noble gases |
What charge does the Halogens family have? Why? |
| -1;because it steals 1 electron to get 8 valence electrons |
| Nonmetals steal electrons from _______ |
| Metals |
| Do nonmetals or metals have a higher ionization energy? |
| Nonmetals |
| What is ionization energy? |
| The energey required to remove an electron from an atom |
| Atomic radius |
| deals with the size |
| Electron affinity |
| Ability of an element to steal electrons |
| Do metals or nonmetals have more electron affinity? |
| Nonmetals |
| Ground state |
| electrons have the least energy and are easily drawn closer to the nucleus |
| Excited state |
| Electrons have the most energy and move farther from the nucleus easily |
| What did Democritus propose about the atom? |
| Said it was indivisible and had different shapes |
| Thomson |
| Discovered electron (called corpucles), conducted cathode ray-tube expiriment, plum-pudding model |
| Milliken |
| Discovered the charge of electrons, oil drop experiment |
| Dalton |
| revised atomic theory, said: atoms could not be created, destroyed, or divided |
| Rutherford |
| Gold foil experiment, discovered that atom was mostly made of empty space |
| Bohr |
| Said electrons were in defind paths and orbits |
| Heisenberg and Shrodinger |
| Revised modern day theory, said electrons in electron clouds. |
| As you go to the right of the periodic table, the ionization energy and electron affinity __________ |
| increases |
As you go _____ the periodic table, the atomic radius/size increases |
| down |
| As you go to the _______ of the periodic table, the size/radius decreases |
| right |
| As you do down the periodic table, the ionization energy and electron affinity _________ |
| decreases |
| Molecular formula |
| The non-simple and complex formula |
| Empirical formula |
| The simplest formula |
| Ammonium |
| NH4+ |
| Hydroxide |
| OH- |
| Nitrate |
| NO3- |
| Acetate |
| C2H3O2- |
| Cyanide |
| CN- |
| Permanganate |
| MnO4- |
| Sulfate |
| SO42- |
| Carbonate |
| CO32- |
| Phosphate |
| PO43- |
| Chlorate |
| ClO3- |
| Nitrite |
| NO2- |
| Chromate |
| CrO4-2 |
| Dichromate |
| Cr2O7-2 |
| Sulfite |
| SO3-2 |
| Chlorite |
| ClO2- |
| Hypochlorite |
| ClO- |
| Perchlorate |
| ClO4- |
| Hydrogen Carbonate |
| HCO3- |
| Hydrogen Sulfite |
| HSO3- |
| Hydrogen Sulfate |
| HSO4- |
| Hydrogen Phosphate |
| HPO4-2 |
| Dihydrogen Phosphate |
| H2PO4- |
IMPORTANT-applies to many things in chemistry
What are the super 7 elements (that form bonds with another atom of their element type)
Ex: X2 <----(this would be a super 7) |
H, Cl, F, O, Br, I, N (all of these would naturally appear like so: H2, Cl2, F2, O2, Br2, I2, N2) |
| Molar mass is measured with the unit ______ |
| grams/mole (g/mole) |
| How would you find the molar mass of anything? |
| You would add up the atomic masses of the individual elements that make it up. |
| Find the molar mass of CaCl2. |
| around 110.98 g/mole |
| How many molecules of O2 are found in 34 moles of O2? |
| 2.05 x 1025 molecules of O2 |
| 30 grams of CaCl2 contains _______ grams of Cl |
around 19.17 grams of Cl How to solve these:
1. Convert the initial quantity into moles (in this case, convert 30 grams of CaCl2 into moles of CaCl2)
2. Find the number of moles of the element that you are trying to find in the compound (in this case, we are tring to find moles of Cl that are in the compound CaCl2)
-do this by looking at the number associated with it in the compound (in this case, the number 2 is along with Cl, so there are 2 moles of Cl in the compound).
3. The number you got in step #2 is not the final answer, you must multiply everything you have done so far, like so (this is for this specific problem):
30 grams of CaCl2 x 1 mole of CaCl2 x 2 moles of Cl 1 110.98 grams CaCl2 1 mole CaCl2
|
Al2(SO4)3 contains ________ moles of Oxygen
(you should not need to calculate anything) |
| 12 moles of Oxygen |
| Find the percent composition of Na in the compound NaH2PO4 |
around 19.17%,
The equation for these kinds of problems is:
Molar mass of element you are trying to find (in this case Na) ? Total molar mass of the compound | | V And then multiply that answer by 100 |
| Convert 25 grams of Fe into molecules of Fe |
| around 2.69 x 1023 molecules of Fe |
How many moles of NaOH are required to form 0.2 moles of Al(OH)3 according to the equation:
3NaOH + AlCl3 = Al(OH)3 + 3NaCl
A) 0.1 mole B) 1 mole C) 3 moles D) 0.6 moles |
D) 0.6 moles Here is the equation for these kinds of problems: 1: Take the intial quantity (in this case, 0.2 moles of Al(OH)3) 2: And then convert it into moles (it is already done for us in this problem, we have it in moles of Al(OH)3 already) 3: Find the number of moles of the element/compound that you are trying to find in the problem (in this case, we are trying to find moles of NaOH) -in order to do this, look at the number in front of the element/compound in the equation (which is a 3 in front of NaOH in this equation, so 3 is the number of moles of NaOH in this equation) 4: That number of moles in step #3 is not the final answer, you must multiply and divide anything you did in this equation so far. I will show this below (this is for this one specific problem): 0.2 moles of Al(OH3) x 3 moles of NaOH = 0.6 moles of NaOH 1 1 mole of Al(OH3) |
1. What is Avagadro's Number? (the quantity)
2. What is it used to measure in Chemistry?
|
1. 6.02 x 1023 2. It is used to measure molecules (or atoms) |
Balance the equation: _H2 + _NO = _H2O + _N2 |
| 2H2 + 2NO = 2H2O + 1N2 |
How many bonds will Nitrogen form (the maximum) You can use your periodic table |
| 3 |
Flourine would try to get 1 bond, why? You can use your periodic table |
| Because it needs 1 more valence electron to have 8 valence electrons (it only has 7 to begin with) |
IMPORTANT-tricky What is the charge of Aluminum? Your periodic tables may help you, but not much
|
| +3 |
Ca is a metal and O is a nonmetal. When the two form bonds with eachother, which one has more control over the valence electrons? A. Ca B. O C. Neither of them have more power over the electrons D. It is almost impossible to conceive which one because every bond is different |
| B. O |
Hydrogen forms _____ bonds (maximum) Why?
|
| 1; because it only needs to make one bond, therefore giving up one electron, with another element in order to have 8 valence electrons |
| What is the SI unit of pressure? |
| Psi (pounds per square inch) |
Pressure is caused by what?
|
| The collisions of particles against walls and eachother. |
| Which two states of matter have pressure? |
| Gas and Liquid |
| What 3 factors can change the pressure of a gas? |
| The amount of gas, the temperature it is at, and the size of the volume in which it is kept in |
1. What is the ideal gas law? 2. What do the variables stand for? 3. What are the units used for each part of it? |
1. PV=nRT
2. (pressure)(volume)=(number of moles)(0.0821)(temp)
3. (atm)(mL)=(moles) (L x atm) (K) K x moles |
| How do you convert °C to K (Kelvin) |
| °C + 273 |
| How do you convert Torr into atm (atmosphere pressure) |
| 760 Torr = 1 atm |
| How do you convert mmHg into atm (atmosphere pressure) |
| 760 mmHg = 1 atm |
1. What is the Combined Gas Law? 2. What are the units used in it? |
1. P1V1 = P2V2 T1 T2
2. YOU CAN USE ANY UNITS!!!! no joke, as long as you use the same ones throughout the entire equation. But temperature (T) MUST be Kelvin (K) |
1. What is the other equation that begins with P = (blank) (blank) ,and includes density in it?
2. What do the variables stand for?
3. What are the units used in it? |
1. P = DRT MM
2. (pressure) = (density)(0.0821)(temp) (molar mass)
3. (atm) = (grams/L) (L x atm) (K) ___________K x mole______ (grams/mole) |
